The equilibrium constant (K_P) for the formation of the air pollutant nitric oxi

Question

The equilibrium constant (K_P) for the formation of the air pollutant nitric oxide (NO) in an automobile engine at 537 degree C is 4.5 Times 10^11. N_2 (g) + O_2 (g) 2NO(g) Calculate the partial pressure of NO under these conditions if the partial pressures of nitrogen and oxygen are 3.00 and 0.012 atm, respectively. Repeat the calculation for atmospheric conditions in which the partial pressures of nitrogen and oxygen are 0.78 and 0.21 atm. and the temperature is 25 degree C. (The K_P for the reaction is 4.0 Times 10^-31 at this temperature.)

Explanation / Answer

N2 (g) + O2 (g) -----> 2 NO (g)
a)
Kp = (pNO)^2/((pN2) * (pO2))
4.5 * 10^-11 = (pNO)^2/(3 * 0.012)
pNO = 1.2728 * 10^-6 atm
b)
Kp = (pNO)^2/((pN2) * (pO2))
4 * 10^-31 = (pNO)^2/(0.78 * 0.21)
pNO = 2.5597 * 10^-16 atm

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